The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
- A
$5.623$
- B
$2.903$
- C
$3.723$
- D
$4.509$
Similar Questions
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.
The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.
Derive the equation of ionization constant $({K_b})$ of weak base.
Derive the equation of ionization constant $({K_b})$ of weak base.
In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$
In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$
What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ - 10}})$
What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ - 10}})$